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Beer-Lambert Law:
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The Beer-Lambert Law describes the relationship between absorbance and the properties of the material through which light is passing. It states that absorbance is directly proportional to the concentration of the absorbing species and the path length of the light through the material.
The calculator uses the Beer-Lambert Law:
Where:
Explanation: The equation calculates the concentration of a solution based on its light absorption properties, molar absorptivity coefficient, and the distance light travels through the sample.
Details: Accurate concentration determination is crucial in analytical chemistry, biochemistry, and environmental science for quantifying substances in solution, monitoring reactions, and ensuring proper formulation of solutions.
Tips: Enter absorbance (dimensionless), molar absorptivity in L/mol·cm, and path length in cm. All values must be valid positive numbers.
Q1: What is the range of validity for the Beer-Lambert Law?
A: The law is valid for dilute solutions where absorbance is typically between 0.1 and 1.0. At higher concentrations, deviations may occur due to molecular interactions.
Q2: What factors can affect accuracy of concentration calculations?
A: Stray light, chemical reactions, fluorescence, scattering, and polychromatic light can all affect the accuracy of absorbance measurements and thus concentration calculations.
Q3: How do I determine the molar absorptivity (ε) for a compound?
A: Molar absorptivity is typically determined experimentally by measuring absorbance of solutions with known concentrations at a specific wavelength.
Q4: Can this calculator be used for any wavelength?
A: Yes, as long as you use the correct molar absorptivity value for the specific wavelength being measured.
Q5: What units should I use for concentration results?
A: The calculator provides results in mol/L (molarity), which is the standard unit for concentration in chemistry applications.